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27FeSO4 🔥→ 8Fe2(SO4)3 + 4Fe2O3 + 3FeS

Decomposition of iron(II) sulfate yields iron(III) sulfate, iron(III) oxide, and iron(II) sulfide (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Thermal decomposition with redox
Thermally decomposable substanceSelf redox agent
🔥
ProductOxidation product + ProductReduction product
Thermal decomposition of oxoacid salt with redox
Oxoacid saltSelf redox agent
🔥
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Decomposition of iron(II) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeSO4Iron(II) sulfate27
Self redox agent
Thermally decomposable
Oxoacid salt

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe2(SO4)3Iron(III) sulfate8
Oxidized
Fe2O3Iron(III) oxide4
Oxidized
FeSIron(II) sulfide3
Reduced

Thermodynamic changes

Changes in standard condition

Decomposition of iron(II) sulfate
27FeSO4Crystalline solid
🔥
8Fe2(SO4)3Crystalline solid + 4Fe2O3Crystalline solid + 3FeSCrystalline solidiron-rich pyrrhotite, α
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
818.0
per 1 mol of
30.30
per 1 mol of
102.3
per 1 mol of
204.5
per 1 mol of
272.7

Changes in aqueous solution

Decomposition of iron(II) sulfate
ΔrG949.2 kJ/mol
K0.51 × 10−166
pK166.29
27FeSO4Crystalline solid
🔥
8Fe2(SO4)3Ionized aqueous solution + 4Fe2O3Crystalline solid + 3FeSCrystalline solidiron-rich pyrrhotite, α
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−1130.0949.2−6944.0
per 1 mol of
−41.85235.16−257.19
per 1 mol of
−141.25118.7−868.00
per 1 mol of
−282.50237.3−1736.0
per 1 mol of
−376.67316.4−2314.7

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
FeSO4 (cr)-928.4[1]-820.8[1]107.5[1]100.58[1]
FeSO4 (ai)-998.3[1]-823.43[1]-117.6[1]
FeSO4 (cr)
1 hydrate
-1243.69[1]
FeSO4 (cr)
4 hydrate
-2129.2[1]
FeSO4 (cr)
7 hydrate
-3014.57[1]-2509.87[1]409.2[1]394.47[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Fe2(SO4)3 (cr)-2581.5[1]
Fe2(SO4)3 (ai)-2825.0[1]-2242.8[1]-571.5[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
FeS (cr)
iron-rich pyrrhotite, α
-100.0[1]-100.4[1]60.29[1]50.54[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

  1. 1